Friday
May 24, 2013

# Search: What mass of CaCl2 is needed to prepare 3.65 L of a 1.75M solution

Number of results: 42,353

Chemistry
You need to re-read the problem and see how impossible it is; however, I think I know what you are asking. You want a 15% solution of CaCl2 but you must use CaCl2.2H2O to make the solution. If that's what you're asking, do it this way. And I'm assuming that is 15 ...
Friday, May 17, 2013 at 4:32pm by DrBob222

chem
How many grams of CaCl2 (molar mass = 111.0 g/mol) are needed to prepare 4.44 L of 0.500 M CaCl2 solution?
Sunday, May 15, 2011 at 7:47pm by jann

chemistry URGENT (1)
(26.4mL)(1.00g/mL) = 26.4g H2O To raise the temperature of 26.4 g H2O by (16.4 C- 10.0 C), we need: (4.18 J/g.C)(26.4 g)(6.4 C) = 706 J needed - 82.8 kJ.mol-1 CaCl2 is equivalent to: 82800 J / 111g CaCl2 = 746 J/g CaCl2 released. Use the values: 706 J needed and 746 J/g CaCl2 ...
Sunday, November 16, 2008 at 2:18pm by GK

Chem
2.00 M = 2.00 mols/Liter of solution. Convert 2.00 M to grams CaCl2 in the solution. 1 L of the solution has a mass of 1.17 x 1000. That is the mass of the water + the mass of the CaCl2. Subtract mass CaCl2 to obtain mass H2O. Now you have the mass and # mols CaCl2 and the ...
Friday, April 25, 2008 at 9:46pm by DrBob222

Chemistry
32% CaCl2 means 32 g CaCl2/100 g soln or 32 g CaCl2 in 68 g water. The moles CaCl2 then is 32g/molar mass CaCl2 molality = moles CaCl2/0.068 kg. delta T = i*Kf*m i = 3. solve for delta T and convert to freezing point.
Tuesday, September 14, 2010 at 6:58pm by DrBob222

chemistry
You need 0.500 x 0.1 = 0.05 moles CaCl2 or 0.05 moles x molar mass CaCl2 = ?? grams CaCl2. Convert ?? g CaCl2 to CaCl2.H2O.
Sunday, September 5, 2010 at 10:54pm by DrBob222

chem
2AgNO3 + CaCl2 ==&gt; 2AgCl + Ca(NO3)2 mole AgCl = 110.5/molar mass = ?? moles CaCl2 used = moles AgCl x (1 mole CaCl2/2 moles AgCl) = ?? M CaCl2 = moles CaCl2/L CaCl2. Solve for L CaCl2 and convert to mL. All of this depends, of course, upon the reaction being complete ...
Monday, November 29, 2010 at 12:29pm by DrBob222

chemistry
34.9 degrees Celsius. 1) convert CaCl2 to moles then multiply it by 82.8kj/mol to find the heat of CaCl2. 2) Use the q=mct equation. Make sure the mass is the TOTAL MASS (of water + CaCl2) 3) Solve. hope this helps! :)
Friday, October 3, 2008 at 11:23pm by sukiyumi

chemistry
Calculate the solubility of Cacl2 in g/L based on the experiement. Given 650g of CaCl2 added to 1.0L and allowed to dissolve as much as possible. While the remaining solid CaCl2 is filtered out of the solution and found to have a mass of 5.509g. What is the solublity of CaCl2
Wednesday, June 6, 2012 at 8:02pm by Greg

Chem
How many moles do you need? That is M x L = mols. Then mol CaCl2 = grams CaCl2/molar mass CaCl2.
Thursday, July 26, 2012 at 9:52am by DrBob222

Chemistry
CaCl2 is the limiting reagent. 1 mole of CaCl2 =2 moles of AgNO3=2 moles of AgCl =1 mole of Ca(NO3)2. 1.50g of CaCl2/110.98 g/mol of CaCl2= number of moles of CaCl2 number of moles of CaCl2*(2 moles of AgCl/1 mole of CaCl2) * 143.32 g of AgCl*mole-1= mass of silver chloride. ...
Wednesday, January 23, 2013 at 5:23pm by Devron

chemistry
I assume the ppt, if done properly, is CaC2O4. Percent CaCl2*2H2O = (mass CaCl2*2H2O/mass sample)*100 = (mass CaCl2*2H2O/0.972 g)*100 = see below. The ppt is CaC2O4. Convert 0.375 g CaC2O4 to moles CaC2O4, then convert to moles CaCl2*2H2O, then to grams CaCl2*2H2O. Plug that ...
Friday, February 19, 2010 at 1:42pm by DrBob222

Chemistry HELP!!!
Only one question, it would be greatly appreciated if you would help me Thanx In an experiment, Na2CO3(aq) was added to 25.0 mL of CaCl2(aq) solution until no more precipitate was formed. The mass of precipitate produced was 2.50 g. Some statements about the experiment follows...
Thursday, September 28, 2006 at 1:24pm by Brittany Rusk

chemistry
This is a basic stoichiometry problem. 1. Write and balance the equation. 2AgNO3 + CaCl2 ==&gt; 2AgCl + Ca(NO3)2 2. Convert what you have, in this case 45 g CaCl2, to moles. moles = grams/molar mass = 45/molar mass CaCl2 = ?? moles CaCl2 3. Using the coefficients in the ...
Thursday, May 13, 2010 at 7:32pm by DrBob222

Chemistry 101 Electrolytes
grams/molar mass = moles CaCl2. 1 mole CaCl2 contains 6.02 x 10^23 molecules CaCl2. There are a total of 3 moles of ions per 1 mole CaCl2. Go from there.
Monday, June 1, 2009 at 5:22pm by DrBob222

chemistry
If 2.1 moles of CaCl2 are dissolved in enough water to make a 0.92-liter solution, what is the resulting molarity? 0.44 M CaCl2 0.70 M CaCl2 2.3 M CaCl2 3.0 M CaCl2
Sunday, November 7, 2010 at 7:31pm by smith

chemistry
Don't let problems like this confuse you. First mols CaCl2 = grams CaCl2/molar mass CaCl2. Then mols Cl^- is twice that.
Saturday, August 4, 2012 at 8:28am by DrBob222

chemistry
What is the mass of 0.425 moles of CaCl2? The molar mass of CaCl2 is 110.98 g/mol.
Friday, February 19, 2010 at 12:09am by Jessica

Chemistry
0.1952 g CaCl2/molar mass CaF2 = 0.002504 mole CaF2. Convert that to moles CaCl2 which is 0.002504. Then concn CaCl2 = mole CaCl2/L soln = ? 0.002504/0.050 L = ??M
Sunday, July 10, 2011 at 9:42am by DrBob222

chemistry
calculate the value of water that is needed to dissolve 1.11 g of CaCl2 in order to prepare a 0.0250 M CaCl2 solution?
Tuesday, July 15, 2008 at 8:26pm by shanta

chemistry
Remember the definitions. Molarity = # mols/L. and # mols = g/molar mass. How many moles CaCl2 do you have in 11.1 g CaCl2. That will be 11.1 g CaCl2/molar mass CaCl2. Then #mols = M x L. You have M and you have mols, calculate L.
Tuesday, July 15, 2008 at 8:26pm by DrBob 222

Chemistry
mols Ca(OH)2 = grams/molar mass = ? mols CaCl2 = mols Ca(OH)2 from the equation (1 mol Ca(OH)2 = 1 mol CaCl2) g CaCl2 = mols CaCl2 x molar mass CaCl2. This is the theoretical yield (TY). The actual yield (AY) is given in the problem as 6.74 g. %yield = (AY/TY)*100 = ?
Monday, October 22, 2012 at 10:58am by DrBob222

science
2 g CaCl2 is how many moles? 2 g/molar mass CaCl2 = ?? moles. M = moles/L = ??moles/0.100 L (that's the 100 mL). M Cl^- is twice that of the CaCl2 since there are two moles Cl^- per mole CaCl2. Post your work if you need further assistance.
Thursday, January 22, 2009 at 5:01pm by DrBob222

Chemistry
I think it would help you if you wrote the equation and balanced it first thing. I assume you can do that. The ppt is CaC2O4 and it has a mass of 0.375. Convert that to moles CaC2O4, then to moles CaCl2.2H2O(using the coefficients in the balanced equation), then to grams CaCl2...
Tuesday, March 23, 2010 at 8:52pm by DrBob222

Chemistry
How many grams of CaCl2 are needed to make 100ml of a 15% solution in water if only the dihydrated (CaCl2 •2H20) salt is available?
Friday, May 17, 2013 at 4:32pm by student123

chemistry
CaCO3 + 2HCl ==&gt; CaCl2 + H2O + CO2 mols CaCO3 = grams/molar mass Convert mols CaCO3 to mols CaCl2 using the coefficients in the balanced equation. g CaCl2 = mols x molar mass.
Wednesday, April 25, 2012 at 4:49pm by DrBob222

Chemistry
I can GUESS that the 23.6 is GRAMS and not mols. I can also GUESS that the next to last sentence should read "when 1 mol calcium chloride dissolves in water?" If my guesses are correct, then q = heat evolved on solution = Cp x delta T. q = 1258 J/oC x delta T for 23....
Thursday, November 1, 2007 at 11:52am by DrBob222

Chemistry
It would have helped if you had posted your work. That way I could find the error. As it is I'm slogging around in the dark. If CaCl2 is exothermic you know the temperature should go up and ot down. 3.80g/molar mass CaCl2 = mols. mols CaCl2 x 82800 = ? Joules. ?J = mass ...
Thursday, June 21, 2012 at 6:56pm by DrBob222

chemisty
Write the equation and balance it. 3CaCl2 + 2Na3PO4 ==&gt; Ca3(PO4)2 + 6NaCl mols Ca3(PO4)2 = grams/molar mass Convert mols Ca3(PO4)2 to mols CaCl2 using the coefficientsin the balanced equation. Then mols CaCl2 = grams CaCl2 x molar mass CaCl2
Thursday, November 29, 2012 at 8:00pm by DrBob222

chemistry
15 g CaCl2/molar mass = mols CaCl2. mols/L = molarity. millimolarity is 1000 times that. % W/V is mass in 100 mL solution.
Friday, February 1, 2008 at 10:00pm by DrBob222

chem
How many moles do you need? M x L = moles. Then moles CaCl2 = grams CaCl2/molar mass CaCl2.
Sunday, May 15, 2011 at 7:47pm by DrBob222

Chemistry
1.Calculate the Theoretical and % Yields of the following equation: 2.What is the limiting and excess reactant? 3.How much excess remains? 2AgNO3 + CaCl2 -&gt; 2AgCl + Ca(NO3)2 mass of 2AgNO3= 1.5g mass of CaCl2= 1.1g (What I have so far): AgNO3: 1.5g(AgNO3) 2mol/170g = 0....
Thursday, January 19, 2012 at 12:50pm by Feloniz

CHEMistry
6.6g AgCl = .046 moles each mole CaCl2 yields 2 moles AgCl, so only 0.023 moles CaCl2 are needed. .023 moles CaCl2 = 2.55g
Monday, November 5, 2012 at 1:10pm by Steve

Chemistry
2.00 M CaCl2 means 2 moles CaCl2/L solution. 1 L of solution has a mass of 1.17 g/mL x 1000 mL = 1170 grams. How much of that is water? 1170 - grams of CaCl2. Convert grams of water to moles. Then moles fraction CaCl2 = moles CaCl2/total moles.
Monday, March 1, 2010 at 1:03pm by DrBob222

chemistry
A 0.972g sample of a CaCl2*2H2O/K2C2O4*H2O solid salt mixture is dissolved in ~ 150ml of deionized water, previously adjusted to a pH that is basic. The precipitate, after having been filtered and air-dried, has a mass of 0.375 g. The limiting reactant in the salt mixture was ...
Friday, February 19, 2010 at 1:42pm by Maria

chemistry
1.30 M = 1.30mols of solute/L of solvent mass of Cacl2 = 1.30 mols CaCl2 x 111g/mol CaCl2(molar mass)= 144.3g of CaCl2 (solute) Solution = 1.11g/ml mass of solution = 1.11g/ml x 1000ml/L x1L = 1110g (solution) mass of solvent = 1110g (solution) - 144.3g (solute)= 965.7g of ...
Tuesday, June 16, 2009 at 4:56pm by ms

chem hwk help!
Given the following reaction: 3 CaCl2 + 2 H3PO4 Ca3(PO4)2 + 6 HCl How many grams of H3PO4 are needed to react completely with 1.837 g of CaCl2? I don't understand at all
Friday, January 25, 2013 at 3:06pm by Annie

chem
mol CaCl2 = grams/molar mass CaCl2. mol CaCl2 x (1 mol Ca/1 mol CaCl2) = ?mol Ca
Wednesday, March 28, 2012 at 10:35pm by DrBob222

Chemistry
The density of H2O=1g/mL, solve for mass. mass=density*volume=(1g/mL)*(500mL)=500g or 0.500 kg m=moles of solute/kg of solvent, solve for moles (0.100 mol/kg)*(0.500 kg)= moles of CaCl2 moles of CaCl2*(111.0g/mole)= mass of CaCl2 ****I'm not Dr. Bob222, but I think this is...
Thursday, March 14, 2013 at 6:48pm by Devron

Chemistry
You need to dissolve CaCl2 in water to make a mixture that is 31.5% calcium chloride by mass. If the total mass of the mixture is 254.6 g, what masses of CaCl2 and water should be used?
Wednesday, January 23, 2013 at 8:37pm by Anon

chem 151
You need to dissolve CaCl2 in water to make a mixture that is 31.5% calcium chloride by mass. If the total mass of the mixture is 419.0 g, what masses of CaCl2 and water should be used?
Saturday, July 7, 2012 at 11:11am by Anonymous

Chemistry
0.315*254.6g= Mass of CaCl2 254.6g-Mass of CaCl2=Mass of H2O
Wednesday, January 23, 2013 at 8:37pm by Devron

chemistry
2 M CaCl2 = 2 mols CaCl2/L soln. 2 mol = 111 x 2 = 222 g (but that's an estimate--you recalculate it). Use density to calculate mass of 1L soln. That will be 1145grams. mass solvent = 1145g-222g = ?g and convert to kg. Then mols Cl in CaCl2 = 4 (2*2) mols Cl in MgCl2 = 10...
Friday, May 10, 2013 at 4:54am by DrBob222

chemistry
Calcium chloride, CaCl2, has been used to melt ice from roadways. Given that a solution is 25% CaCl2 by mass, estimate the freezing point.
Monday, December 20, 2010 at 9:33am by Akkam

chemistry
2AgNO3 + CaCl2 ==&gt; 2AgCl + Ca(NO3)2 moles CaCl2 = M x L = ?? moles AgCl produced is 2x moles CaCl2 = ?? g AgCl = moles AgCl x molar mass AgCl.
Wednesday, September 29, 2010 at 2:22am by DrBob222

Chemistry
If the molality of a CaCl2 solution is .100 mol/kg, and was made from 500.0 mL of water, how many grams of CaCl2 were needed to make the solution? Step by step would be appreciated!
Thursday, March 14, 2013 at 6:48pm by Tim

Chemistry
A .972g sample of a Cacl2 2H2O/K2C2O4 H2O solid salt mixture is dissolved in 150 ml of deionized water, previously adjusted to a pH that is basic . The precipitate after having been filtered and air dried has a mass of .375g. what is the percent by mass of CaCl2 2H2O
Tuesday, March 23, 2010 at 8:52pm by Ann

Chemistry
What volume of .300 M CaCl2 is needed to react completely with 40.00 Ml of .200 M H2PO4. according to the following equation 3 CaCl2 (aq) + 2 H3PO4 (aq)-&gt; Ca3(po44)2 + 6 HCL (aq)
Tuesday, June 7, 2011 at 7:29pm by Vinny

chemistry
Molarity=moles/volume (L)=0.015= x moles/7.25 L Solve for moles, 0.015*7.25L= moles of CaCl2 in solution moles of CaCl2 in solution*(110.98 g/mol)= mass of CaCl2 in g.
Friday, March 15, 2013 at 1:30pm by Devron

chemistry
If this is 10% by mass (w/w) you can't do it unless you know the density. Is this 10% w/w or 10% w/v? If 10% w/v, which I suspect, convert 10 g CaCl2 to CaCl2.10H2O and that many g in 100 mL will be 10% CaCl2. You need 250 mL; therefore, you will need 2.5 times that amount.
Sunday, September 5, 2010 at 11:00pm by DrBob222

Chemistery
How many mols in 2 g CaCl2? 2 g x (110.98 g CaCl2/1 mol CaCl2) = ?? mols M = # mols/L = ??mols/0.100 L = xx molar. There are two mols Cl^- per 1 mol CaCl2; therefore, (Cl^-) is twice that for CaCl2.
Tuesday, January 20, 2009 at 11:22pm by DrBob222

Chemistry
If 10.0g of CaCl2 and 10.0g of NaCl are dissolved in 100.0mL of solution, what is the concentration of chloride ions? I found the molar mass of CaCl2 is 111.0g/mol; the molar mass of NaCl is 58.44g/mol. I divided 10g CaCl2/111.0g CaCl2 I divided 10g NaCl/588.44g NaCl and added...
Monday, July 12, 2010 at 9:33am by Casey

chemistry
pi = iMRT i = 3 for CaCl2 moles = grams/molar mass CaCl2, then M = moles/L R = 0.08206 T = 20 in kelvin.
Thursday, September 29, 2011 at 2:57pm by DrBob222

chemistry
A chemist wants to make 5.5 L of a 0.250 M CaCl2 solution, what mass of CaCl2 (in g) should the chemist use?
Saturday, November 20, 2010 at 1:07pm by Lisa

Chemistry
A chemist wants to make 4.5 L of a 0.310 M CaCl2 solution what mass of CaCl2 (in g) should the chemist use
Monday, November 1, 2010 at 7:40pm by Lisa

Chemistry
How many moles do you have in 100 mg CaCl2? moles = grams/molar mass. Then there are 2 Cl atoms/molecule of CaCl2.
Wednesday, February 17, 2010 at 1:09pm by DrBob222

Chemistry 104
What mass (in grams) of calcium carbonate is needed to react completely with 73 mL of 0.10 M HCl according to 2HCl + CaCO3 --&gt; CaCl2 + H20 + CO2?
Thursday, November 11, 2010 at 3:29pm by Brenna

Chemistry
23.7/molar mass CaCl2 = moles CaCl2 moles Cl^- = 2 times that. Convert 3675 g water to liters using the density. Then M = mols/L.
Sunday, September 26, 2010 at 12:53pm by DrBob222

chimistry
3.24 moles of Cl2 will, in the right kind of reaction, produce the equivalent of 3.24 moles of CaCl2. 1 mole of CaCl2 has a mass of ?? grams (look up the molar mass). Therefore, 3.24 moles should be ?? grams.
Thursday, February 18, 2010 at 10:10pm by DrBob222

Chemistry
Note the reaction produces 81.5 kJ energy per 1 mol CaCL2. Convert that to kJ/1 g CaCl2. q = mass x speific heat water x (Tf-Ti). mass = 14.0 sp.h. water is in the problem. Tf is final T Ti is initial T.
Saturday, November 10, 2007 at 10:08am by DrBob222

Chemistry
You're on the right track but you have your numbers a little mixed up. moles = grams/molar mass. moles AgNO3 = 1.5/170 = 0.00882 0.00882 moles AgNO3 x (2 mol AgCl/2 mol AgNO3) = 0.00882 mol AgCl produced (trial). moles CaCl2 = 1.1/111 = 0.00991 You used the wrong molar ...
Thursday, January 19, 2012 at 12:50pm by DrBob222

camestry
Calculate the number of grams of calcium chloride (CaCl2) needed to react with excess silver nitrate (AgNO3) to produce 6.60 g of silver chloride (AgCl). The equation for the reaction is given below: CaCl2 + 2AgNO3 &#8594; 2AgCl + Ca(NO3)2
Monday, November 5, 2012 at 1:10pm by mohammed

chemistry
What mass (in grams) of CaCl2(s) must be dissolved in pure water at 10.0 deg Celsius to make a 26.4 mL solution and to increase the solution temperature to 16.4 deg Celsius? Assume that there is no heat loss from the solution and that the solution has the same physical ...
Sunday, November 16, 2008 at 3:43am by Anonymous

chemistry URGENT (1)
What mass (in grams) of CaCl2(s) must be dissolved in pure water at 10.0 deg Celsius to make a 26.4 mL solution and to increase the solution temperature to 16.4 deg Celsius? Assume that there is no heat loss from the solution and that the solution has the same physical ...
Sunday, November 16, 2008 at 2:18pm by Anonymous

Chemistry
If 10.0g of CaCl2 and 10.0g of NaCl are dissolved in 100.0mL of solution, what is the concentration of chloride ions? (the molar mass of CaCl2 is 111.0g/mol; the molar mass of NaCl is 58.44g/mol. I found individual molar mass of: Ca-40.08 Cl-35.45 Na-22.99 So I divided 10g ...
Sunday, July 11, 2010 at 12:57pm by Casey

Chemisty
Use stoichiometry to back calculate from 5.3 g CaCl2 to see the moles HCl used (you could go the long way and calculate moles CaCO3 used then convert to HCl but that step isn't necessary). moles CaCl2 = grams/molar mass = 5.3/about 111 = about 0.048 (but you need to do it ...
Sunday, November 20, 2011 at 8:22pm by DrBob222

Chemistry
You're ok for part of it. 0.270 mol CaCO3 is right. 0.384 mol HCl is right. But you will not form 0.170 mol CaCl2. You have LR of HCl but you must have arrived at that answer incorrectly. Convert mols CaCO3 to mols CaCl2 by 0.270 x (1 mol CaCl2/1 mol CaCO3) = 0.270. ...
Wednesday, October 3, 2012 at 12:39am by DrBob222

chemistry
A solution is prepared by dissolving 23.7 g of CaCl2 in 375 g of water. The density of the resulting solution? is 1.05 g/ml. the concentration of CaCl2 is ________% by mass. answer: 5.94 can someone tell me the steps?
Wednesday, September 15, 2010 at 5:39pm by john

Shawn
How many milliliters of 0.355 M NaF solution are needed to react completely with 24.6 mL of 0.216 M CaCl2 solution? How many grams of CaF2 will be formed? The reaction is CaCl2(aq) + 2NaF(aq) &#8594; CaF2(s) + 2NaCl(aq)
Friday, July 8, 2011 at 3:06pm by Chemistry

Chem hwk
3CaCl2 + Al2(SO4)3 ==&gt; 3CaSO4 + 2AlCl3 mols CaCl2 = grams/molar mass Convert mols CaCl2 to mols CaSO4 using the coefficients in the balanced equation. Convert mols CaSO4 to g. g = mols x molar mass.
Monday, January 28, 2013 at 2:58pm by DrBob222

chemistry
The hydrated CaCl2 is just dehydrated. CaCl2.2H2O + heat --&gt; CaCl2(s) + 2H2O(g)
Monday, June 14, 2010 at 2:47pm by DrBob222

chemistry
Ca(ClO3)2 + KCl --&gt; CaCl2 + 3O2 + KCl Mass of test tube = 7.918g Mass of KCl/Ca(ClO3)2 mixture + tube = 19.164g Mass of KCl/CaCl2 residue + tube = 18.635g What is the weight % of Ca from the Ca(ClO3)2 impurity in the original mixture?
Wednesday, February 11, 2009 at 4:01am by kevin

Chemistry
Na2CO3 + CaCl2 ==&gt; CaCO3 + 2NaCl The Law of conservation of mass says that the mass on the left = mass on the right.
Tuesday, September 25, 2012 at 10:31pm by DrBob222

chemistry
There are 2 moles Cl ions/1 mole CaCl2; therefore, moles CaCl2 = (M x L)/2 moles = grams/molar mass Solve for grams.
Tuesday, December 14, 2010 at 11:17pm by DrBob222

chemistry
Change 3.60 g CaCl2 to moles; moles = grams/molar mass (-82,800 J/mol x moles CaCl2) + [moles H2O x specific heat water(J/mol) x (Tfinal-Tinitial)] = 0 Check my thinking.
Thursday, October 20, 2011 at 3:01pm by DrBob222

Chemistry
a 110 g solid sample that is a mixture of CaCO3 and CaCl2 is reacted with 1.50 L of 1.45M HCl. Of the calcium salts, only calcium carbonate reacts with HCl- the reaction forms CaCl2 and CO2. The excess/unreacted HCl requires 0.850 L of 0.543 M NaOH to titrate it to the ...
Monday, December 3, 2012 at 10:31pm by Cristian

chemistry
A 2.33-g sample of a mixture of CaCl2 and Ca(NO3)2 is treated with excess AgNO3(aq). The precipitate is filtered off, dried and weighed. The dried precipitate weighs 3.9 g. What is the percentage by mass of CaCl2 in the original mixture?
Sunday, October 7, 2012 at 7:37pm by Kevin

Chemistry
mols CaCo3 = grams/molar mass. mols HCl = grams/molar mass. Convert mols CaCO3 to mols CaCl2 using the coefficients in the balanced equation. Do the same for mols HCl. It is likely that these two values for mols CaCl2 will not be the same which means one is not right; the ...
Wednesday, December 19, 2012 at 10:46pm by DrBob222

Gen Chemistry
Convert 3.9565 g Ca3(PO4)2 to moles, then to moles CaCl2, then M = moles CaCl2/L CaCl2.
Saturday, December 11, 2010 at 9:06pm by DrBob222

Chemistry
This is a Lab Stoichiometry and Gravimetric Analaysis Balance equation: Na2CO3 + CaCl2 ---&gt; CaCO3 + 2NaCl Precipitate(?): Not Sure Na2CO3 + CaCl2 Calculate the mass of the dry precipitate and the number of moles of precipitate produced ine the reactation? Empirical ...
Sunday, October 28, 2007 at 5:13pm by Monte;

chemistry
Please note the correct spelling of Celsius. How much heat does the CaCl2 add to the water? That is 7.2 g (1 mol/molar mass CaCl2) x (82,800 Joules/mol). Then q = mass water x specific heat water x (Tf-Ti) where Tf is the final T and Ti is the initial T. Most dilute solutions ...
Friday, October 3, 2008 at 11:23pm by DrBob222

Chemistry
mols CaCl2 = grams/molar mass Substitute and solve for mols. molality = mols/kg solvent Substitute and solve for m. Then delta T = i*Kb*m i = 3 for CaCl2.
Thursday, March 7, 2013 at 1:54pm by DrBob222

Chemistry
Urgent... Someone please help!! Can someone please check to see if I am doing these correctly, I have a test tomorrow... Thank you :) Q) Calculate the new molarity of a 35mL sample of 0.450 M CaCl2 solution that is diluted with enough water to make 250 mL of solution. A) 0.450...
Tuesday, April 2, 2013 at 8:19pm by Kishwa

Chemistry
1.72% w/v means 1.72 g CaCl2 in 100 mL of solution so that would be 10x that for 1 L of solution or 17.2 g CaCl2. The answer to the problem, therefore, is 17.2 g CaCl2 but it makes a difference how the solution is prepared. You can NOT add 17.2 g CaCl2 to a liter (1000 mL) of ...
Wednesday, April 27, 2011 at 5:29pm by DrBob222

Chemistry/maths
Using the following stock solutions: NaCl, 100mmol KCl, 200mmol CaCl2, 160mmol Glucose, 5mmol Calculate the volumes of each stock solution and the volume of water needed to prepare 100ml of a single solution containing NaCl at 5.0mmol KCl at 2.5mmol CaCl2 at 40mmol Glucose at ...
Thursday, October 22, 2009 at 8:35am by jess

Chemistry
158.5 mL of a AgNO3 solution at 5.0M was combined with a 3.5M CaCl2 solution. 110.5g of AgCl was recovered. Given that the CaCl2 is the limiting reagent, how many milliliters of the 3.5M CaCl2 solution was used?
Tuesday, April 5, 2011 at 6:39am by Sara

Science
first, identify the reactions: KCl + AgNO3 = KNO3 + AgCl CaCl2 + 2AgNO3 = Ca(NO3)2 + 2AgCl convert grams to moles for KCl and CaCl2 to get total moles of Cl involved Each mole of Cl requires one mole of AgNO3 to react. divide that no. of moles by 1.57 to get liters of AgNO3 ...
Friday, October 19, 2012 at 2:31pm by Steve

chem hwk help!
cmon, we just did one of these. convert grams to moles, then use the reaction to figure the relative amounts needed/produced. moles of input = 1.837/111 = .01655 moles CaCl2 Each 3 CaCl2 requires 2 H3PO4 so, 2/3 * .01655 = .011 moles H3PO4 .011 moles H3PO4 = .011 * 98 = 1.081g
Friday, January 25, 2013 at 3:06pm by Steve

chem
158.5 mL of a AgNO3 solution at 5.0M was combined with a 3.5M CaCl2 solution. 110.5g of AgCl was recovered. Given that the CaCl2 is the limiting reagent, how many milliliters of the 3.5M CaCl2 solution was used? 2 sig figs
Monday, November 29, 2010 at 12:29pm by Michelle

chemistry
2Na3PO4 + 3CaCl2 ----&gt; Ca3 (PO4)2 + 6NaCl how many moles of CaCl2 remain if .10 mol Na3PO4 and .40 mol CaCl2 are used? When amounts of both materials are listed one must worry about which is the limiting reagentalthough the problem seems to suggest that Na3PO4 is the ...
Wednesday, June 21, 2006 at 6:14pm by Hawk

Chemistry
I would really aprreciate if someone could help me, thank you so much. The white limestone cliffs of Dover, England, contain a large percentage of calcium carbonate(CaCO3). A sample of limestone weighing 84.4g reacts with an excess of hydrochloric acid to form calcium chloride...
Monday, July 9, 2007 at 10:24pm by Amy

Chemistry
I expect if I look really hard I could find exactly where you went off track but it is easier to show you how to do the problem. Plan: Determine molarity CaCl2 and molarity NaCl, then multiply M CaCl2 by 2 (to find M Cl) and add to molarity NaCl. mols CaCl2 = 10/111 = 0.09 M...
Sunday, July 11, 2010 at 12:57pm by DrBob222

Chemistry
1. Convert 20.8 g CaCl2 to moles (Diveide by the formula mass of CaCl2). 2. The heat given off is: &#8710;H(sln) = (1258 J/°C)(37.1°C - 25.0°C) 3. Divide the answer in step #2 by the answer in #1 to get the joules/mole. This value is negative since the heat is ...
Saturday, October 18, 2008 at 10:37pm by GK

Chemistry
You need to know the grams (or moles) of CaCl2 needed to produce a change of x joules.
Monday, March 7, 2011 at 8:47am by DrBob222

AP Chemistry
a)CaCl2 b)water c)CaCl2 d)water e)CaCl2
Wednesday, November 24, 2010 at 12:50am by Anonymous

AP Chemistry
a)Water b)CaCl2 c)CaCl2 d)Water e)CaCl2
Wednesday, November 24, 2010 at 12:50am by Sean

chemistry
What's the density of 10%CaCl2? You would want 30 g CaCl2/300 g soln but that isn't 300 mL. That would be 300 g CaCl2 in 270 g H2O and that will produce a volume that is probably about 280 mL.
Tuesday, November 29, 2011 at 12:34pm by DrBob222

Chemisty
From the valences or the oxidation states. Na in NaCl is +1. Cl is -1. CaCl2 will have Ca+2 and 2 Cl^- so CaCl2 will be more effective than NaCl. (NaCl will cause coagulation, too, but it won't be as effective as CaCl2). K3PO4 is 3K+ and 1 PO4^-3. I will leave Fe2(SO4)3 ...
Monday, February 11, 2008 at 6:42pm by DrBob222

chemistry
I assume you meant hydrochloric acid or aqueous hydrogen chloride (hydrogen chloride is a gas and there would be little to no reaction between the gas and solid CaCO3). Here is a step by step. Print this out so you can keep it. It will work all of your stoichiometry problems ...
Wednesday, August 15, 2012 at 7:26pm by DrBob222

chemistry
How do you sole this problem: how many grams of CaCl2 are needed to prepare 7.25 L of .015M solution?
Friday, March 15, 2013 at 1:30pm by Brittany jones

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